The question is in the picture ### Chemical Reactions: Balancing Equations**K** = \( \frac{[\text{C}_4 \text{H}_{10} \text{O}]}{P_{\text{C}_4 \text{H}_{10} \text{O}}} \)**Problem Statement:**b) Carbon monoxide gas is oxidized with oxygen gas to form carbon dioxide gas.**Question:**Choose the correct balanced net ionic equation (simplest whole-number coefficients) for this reaction.**Options:**- \( \text{CO}(l) + \text{O}_2(g) \rightarrow \text{CO}_2(g) \)- \( 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \)- \( \text{CO}(g) + 2 \text{O}(g) \rightarrow \text{CO}_2(g) \)- \( \text{CO}(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) \)**Additional Interface:**- A "Submit" button appears below the question options for user interaction.### Explanation:To solve this, we need to find the simplest whole-number coefficients to balance the given chemical equation.The correct balanced equation is:\[ 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \]This equation shows that two molecules of carbon monoxide gas react with one molecule of oxygen gas to produce two molecules of carbon dioxide gas, ensuring that the number of atoms for each element is equal on both sides of the equation.**Note:**There are no graphs or diagrams accompanying this problem. Ensure to click the "Submit" button after selecting your answer to proceed.

Let the reaction is x CO (g) + y O2 (g) → z CO2(g) Let, x=2 Number of carbon atom on left-hand…

Carbon monoxide gas is oxidized with oxygen gas to form carbon dioxide gas. Choose the correct balanced net ionic equation (simplest whole-number coefficients) for this reaction. O co() - 0,(g) = CO2(g) O 2c0(g) + 02(g)= 2CO2(g) O co(g) + 20(g) = CO2(g) O co(g) + O2(g) =CO2(g)

Carbon monoxide gas is oxidized with oxygen gas to form carbon dioxide gas. Choose the correct balanced net ionic equation (simplest whole-number coefficients) for this reaction. O co() - 0,(g) = CO2(g) O 2c0(g) + 02(g)= 2CO2(g) O co(g) + 20(g) = CO2(g) O co(g) + O2(g) =CO2(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

The question is in the picture

### Chemical Reactions: Balancing Equations

**K** = \( \frac{[\text{C}_4 \text{H}_{10} \text{O}]}{P_{\text{C}_4 \text{H}_{10} \text{O}}} \)

**Problem Statement:**
b) Carbon monoxide gas is oxidized with oxygen gas to form carbon dioxide gas.

**Question:**
Choose the correct balanced net ionic equation (simplest whole-number coefficients) for this reaction.

**Options:**
- \( \text{CO}(l) + \text{O}_2(g) \rightarrow \text{CO}_2(g) \)
- \( 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \)
- \( \text{CO}(g) + 2 \text{O}(g) \rightarrow \text{CO}_2(g) \)
- \( \text{CO}(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) \)

**Additional Interface:**
- A "Submit" button appears below the question options for user interaction.

### Explanation:

To solve this, we need to find the simplest whole-number coefficients to balance the given chemical equation.

The correct balanced equation is:
\[ 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \]

This equation shows that two molecules of carbon monoxide gas react with one molecule of oxygen gas to produce two molecules of carbon dioxide gas, ensuring that the number of atoms for each element is equal on both sides of the equation.

**Note:**
There are no graphs or diagrams accompanying this problem.

Ensure to click the "Submit" button after selecting your answer to proceed.

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